Iron(III) nitrate. Fe(NO_3)_3, dissolves in water to produce Fe^+3 and NO^-_3 io

Question

Iron(III) nitrate. Fe(NO_3)_3, dissolves in water to produce Fe^+3 and NO^-_3 ions. Sodium salicylate, NaC_7H_5O_3, dissolves in water to produce Na^+ and C_7H_5O^-_3 (salicylate) ions. When solution of Fe(NO_3)_3 and NaC_7H_5O_3 are mixed, the Fe^+3 and C_7H_5O^-_3 ions react to form a reddish-purple material having the formula [FeC_7H_5O_3]^+2. The reaction between the Fe^+3 and C_7H_5O^-_3 ions is fast and reversible and reached the equilibrium quickly. (a) Write a balanced molecular equation for the above reaction. (b) Write the net ionic equation for the reaction in above question. (c) The intensity of reddish-purple color increases over the time. What can you conclude from this result? (d) Suppose that the product (FeC_7H_5O_3]^+2 was not very soluble in water. Would this tend to make the reaction move more in the forward or backward direction? Explain.

Explanation / Answer

For the given reaction,

(a) Balanced equation,

Fe(NO3)3 + 3NaC7H5O3 ---> Fe(C7H5O3)^2+ + 3NaNO3 + 2C7H5O3-

(b) net ionic equation,

Fe3+ + C7H5O3- --> Fe(C7H5O3)^2+

(c) The intensity is directly proportional to the amount of Fe(C7H5O3)^2+ present in solution which increases over time and forward reaction proceeds. Thus intensity goes up with time.

(d) If the final product is not very soluble in water. This would tend to make the reaction move in the forward direction as the concentration of Fe(C7H5O3)^2+ would be lower in solution and to establish equilibrium more of Fe3+ and C7H5O3- would react.

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